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What is the volume in liters of 15.0 kg CO2 at STP?
The molar mass of CO2 is 44.01 g/mol. Using the ideal gas law, we can calculate the number of moles of CO2 in 15.0 kg (15000 g). At STP conditions, 1 mole of gas occupies 22.4 L, so once you find the number of moles, you can convert that to liters.
What is the density of carbon dioxide CO2 at STP if 1 mole occupies 22.4 L Report answer in grams per liter gL?
Density of CO2 at STP = 44.01 g/mol divided by the 22.4 liters. 1.96 grams/Liter
If 1.00 kg of Fe2O3 completely reacts with CO the volume of CO2 released at STP will be?
There are several different possible reactions of Fe2O3 with CO, depending on temperature and ratio of reactants. The simplest is probably Fe2O3 + CO ==>2FeO + CO21.00 Kg x 1000 g/Kg x 1 mole Fe2O3/160 g = 6.25 moles Fe2O3 moles CO2 produced = 6.25 moles CO2 Volume CO2 at STP = 6.25 moles x 22.4 L/mole = 140 Liters
what would be the volume of CO2 (at STP) produced from the complete reaction of 10 grams of CaCO2?
Assuming complete reaction, the molar mass of CaCO3 is approximately 100.09 g/mol. One mole of CaCO3 produces one mole of CO2. Therefore, 10 grams of CaCO3 will produce approximately 2.24 liters of CO2 at STP (22.4 L/mol).
Identify the limiting reagent and the volume of CO2 formed when 11 L CS2 reacts with 18 L O2 to produce CO2 gas and SO2 gas at STP. CS2(g) plus 3O2(g) and rarr CO2(g) plus 2SO2(g)?
To determine the limiting reagent, we need to compare the amount of CO2 that could be produced from each reactant. First, convert the volumes to moles using the ideal gas law. Then, use the coefficients from the balanced chemical equation to find the amount of CO2 that each reactant could produce. The limiting reagent is the one that produces the least amount of CO2. The volume of CO2 formed can be calculated using the stoichiometry of the limiting reagent.
What is the volume of 10 grams of CO2 at STP?
At standard temperature and pressure (STP), which is defined as 0 degrees Celsius and 1 atmosphere pressure, the volume of 10 grams of CO2 can be calculated using the ideal gas law. The molar mass of CO2 is 44.01 g/mol. Using the ideal gas law equation, you can determine the volume to be approximately 4.48 liters.
When calcium carbonate is heated strongly carbon dioxide gas is released CaCO3CaO CO2 what is the volume of CO2 measured stpis produced if 15.2 grams of caco3 is heated?
The molar mass of CaCO3 is 100.09 g/mol, and the molar mass of CO2 is 44.01 g/mol. By using stoichiometry, you can calculate that 15.2 grams of CaCO3 would produce 6.51 grams of CO2. Using the ideal gas law, you can then convert the mass of CO2 to volume using its molar volume at STP (22.4 L/mol). The volume of CO2 produced would be around 3.32 liters.
What is the volume in liters of 15.0 kg CO2 at STP?
The molar mass of CO2 is 44.01 g/mol. Using the ideal gas law, we can calculate the number of moles of CO2 in 15.0 kg (15000 g). At STP conditions, 1 mole of gas occupies 22.4 L, so once you find the number of moles, you can convert that to liters.
How do i solve this at constant pressure and temperature 30g of CO2 gas occupies a volume of 410mL. Determine the volume of 110g of CO2 in liters?
Under these conditions, the volume will be directly proportional to the number of moles. And the number of moles varies with the number of grams. 110 g/30 g = 3.67, so there are 3.67 x more moles in 110 g as there are in 30 g. And the volume will be 3.67 x greater or 3.67 x 410 ml = 1503 ml = 1.5 liters (to 2 significant figures)
What volume will 15 g of NH3 occupy at stp?
The volume of ammonia is 19,5 L.
What is the density of carbon dioxide CO2 at STP if 1 mole occupies 22.4 L Report answer in grams per liter gL?
Density of CO2 at STP = 44.01 g/mol divided by the 22.4 liters. 1.96 grams/Liter
What is the volume of 11 g of SO2 at STP conditions?
At STP conditions (standard temperature and pressure), the volume occupied by 1 mole of ideal gas is 22.4 liters. Since the molar mass of SO2 is approximately 64 g/mol, 11 g of SO2 is about 0.172 moles. Therefore, the volume of 11 g of SO2 at STP would be approximately 3.85 liters.
what volume in milliliters will 0.00922 g of H2 gas occupy at STP?
0.00922 g of H2 gas will occupy approximately 0.100 L at STP
If 1.00 kg of Fe2O3 completely reacts with CO the volume of CO2 released at STP will be?
There are several different possible reactions of Fe2O3 with CO, depending on temperature and ratio of reactants. The simplest is probably Fe2O3 + CO ==>2FeO + CO21.00 Kg x 1000 g/Kg x 1 mole Fe2O3/160 g = 6.25 moles Fe2O3 moles CO2 produced = 6.25 moles CO2 Volume CO2 at STP = 6.25 moles x 22.4 L/mole = 140 Liters
what would be the volume of CO2 (at STP) produced from the complete reaction of 10 grams of CaCO2?
Assuming complete reaction, the molar mass of CaCO3 is approximately 100.09 g/mol. One mole of CaCO3 produces one mole of CO2. Therefore, 10 grams of CaCO3 will produce approximately 2.24 liters of CO2 at STP (22.4 L/mol).
What is the volume occupied by 0.155 g of boron trifluoride at stp?
The ideal gas law states that at STP (Standard Temperature and Pressure), one mole of gas occupies 22.4 L of volume. Boron trifluoride (BF3) has a molar mass of 67.8 g/mol. Therefore, 0.155 g of boron trifluoride is 0.155/67.8 = 0.00228 moles. At STP, this amount of boron trifluoride would occupy 0.00228 * 22.4 = 0.051072 L of volume.
What is the density of CO2 gas at STP?
The density of CO2 gas at standard temperature and pressure (STP) is approximately 1.977 g/L. This value is derived from the molar mass of carbon dioxide (44.01 g/mol) divided by the molar volume at STP (22.4 L/mol). The calculation is as follows: 44.01 g/mol / 22.4 L/mol = 1.977 g/L. This density value is useful in various applications, such as in gas laws and stoichiometry calculations.
